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Lone pairs typically have the greater repulsion because lone pairs want to be as far apart from one another as possible, even more so than bonding pairs. This is because the lone pairs consist of free-moving electrons.

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Q: What has the strongest repulsion bonding pairs or lone pairs?
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How does a lone pair distort the molecular shape?

A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.


Why the lone pair-lone pair repulsion is more than bond pair-bond pair?

In bonded pairs of electrons the repulsion of the negative charges is somewhat reduce by the positive charge of the bonded atom's nucleus. Lone pairs do not have this.


What are lone pairs in bonding?

because they are not paired....


Why is the water bond angle 104.5 less than the CH4 bond angle 109.5?

in water there are two bond pairs and two lone pairs where as in CH4 there are are four bond pairs nad no lone pair. in ch4 there is only bond pair to bond pair repulsion but in water there are three types of repulsions, lone to lone (greatest repulsion), lone to bond ( lesser repulsion ) and bond to bond ( the least repulsion) , therefore due to the presence of two lone pairs in water the bond pairs are repelled with greater force and they get compressed, reducing the ideal bond angle from 109.5 to 104.5 on the other hand, ch4 has only bond pairs and they dont repel each other that strongly so its angle is greater n its 109.5..


How many lone pairs of electrons are there in the ClO3- ion?

Chlorine (nucleus) has 1 lone pair and 3 polar-covalent bonding pairs (the shared pairs with O). Each oxygen (nucleus) has 3 lone pairs and 1 polar-covalent bonding pair (the shared pair with Cl)

Related questions

Why does the repulsion between lone pairs are stronger than the repulsion between bonding pairs or between one bonding pair and a lone pair?

The repulsion between lone pairs are stronger than the repulsion between bonding pairs between one bonding pair and lone pair due to electrostatic interactions.


What is the bond angle of C2H4Cl2?

it's nearly 118.because it has three pair of electron,two bonding pairs and a lone pair.the repulsion between lone pair and bonding pairs is more than the repulsion between bonding pair and bonding pair.so the angle of the bond is 2 degree less than a trigonal planar with 3 bonding pairs (120).


How does lone pairs distort the molecular shape?

A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.


How does a lone pair distort molecular shape?

A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.


How does a lone pair distort a molecular pair?

A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.


How does a lone pair distort the molecular shape?

A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.


How does electron repulsion determine molecule shape?

Because they push the bonding pairs down. For example in a water molecule, it has 2 lone pairs which push the 2 bonding pairs down to form a V-shaped molecule. Hope this helps


What does the vsepr theory explain for covalent bonds?

VSEPR theory explains the geometry around a central atom in terms of repulsion beween pairs of electrons, pairs involved in bonding and lone pairs.


Should BH3 and NH3 have the same shape?

NH3's shape is trigonal pyramidal, which has 1 e lone pairs and 3 bonding pairs, while BH3's shpe is trigonal planar, with 0 e lone pair and 3 bonding pairs. It's the force that electron lone pairs exert that pushes the molecules further and the repulsion force of lone pairs that aided in changing the shape of the molecules. Hence, the shape are different ...


How are the shapes of molecules of polyatomic ions related to the number of electron pairs surrounding the central atom?

VSEPR theory predicts that the electron pairs in bonds and lone pairs repel one another and this gives rise to the shape. Lone pairs repel bonding pairs more than bonding pairs repel one another. It is often taught that electrostatic repulsion is the major cause of this but the man who invented the theory, Prof. Gillespie, says that the repulsion is due to the Pauli Exclusion Principle. See wikipedia link for a reasonable description.


How many lone pair and bonding pair in phosphine?

3 bond pairs and no lone pairs


Why the lone pair-lone pair repulsion is more than bond pair-bond pair?

In bonded pairs of electrons the repulsion of the negative charges is somewhat reduce by the positive charge of the bonded atom's nucleus. Lone pairs do not have this.